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Chapter 15: Problem 74

True or false? The acidity of a given volume of 1.0 \(\mathrm{M}\) hydrofluoric acid is the same as that of the same volume of \(1.0 \mathrm{M}\) hydrochloric acid. Explain your answer.

Short Answer

Expert verified
False. The acidity of a given volume of 1.0 M hydrofluoric acid is not the same as that of the same volume of 1.0 M hydrochloric acid. This is because HCl is a strong acid and completely dissociates in water, producing a 1.0 M concentration of H+ ions, whereas HF is a weak acid and only partially dissociates, resulting in a lower H+ ion concentration.

Step by step solution

01

Understanding the dissociation of acids in water

When an acid dissolves in water, it donates a hydrogen ion (H+) or proton to the water, forming hydronium ions (H3O+). This process is called dissociation. The strength of an acid is determined by its ability to donate protons to water. Strong acids, like HCl, completely dissociate in water, releasing H+ ions. On the other hand, weak acids like HF only partially dissociate, releasing fewer H+ ions.
02

Comparing the dissociation of hydrofluoric acid (HF) and hydrochloric acid (HCl)

Both hydrofluoric acid (HF) and hydrochloric acid (HCl) dissolve in water, donating H+ ions and forming their respective anions (F- and Cl-). The difference lies in their ability to dissociate in water. HCl is a strong acid, meaning it completely dissociates in water: \[HCl_{(aq)} \rightarrow H^+_{(aq)} + Cl^-_{(aq)}\] In contrast, HF is a weak acid, meaning it only partially dissociates in water: \[HF_{(aq)} \rightleftharpoons H^+_{(aq)} + F^-_{(aq)}\] Because HF is a weak acid, the concentration of H+ ions released in the solution will be lower than that for HCl.
03

Comparing the acidity of 1.0 M hydrofluoric acid and 1.0 M hydrochloric acid

Since HCl completely dissociates in water, a 1.0 M solution of HCl would also have a concentration of H+ ions equal to 1.0 M. On the other hand, since HF only partially dissociates in water, a 1.0 M solution of HF would have a lower concentration of H+ ions than 1.0 M.
04

Conclusion

From the comparison of the dissociation of HF and HCl and the concentrations of H+ ions released in the solutions, it can be concluded that the acidity of a given volume of 1.0 M hydrofluoric acid is not the same as that of the same volume of 1.0 M hydrochloric acid. The statement is, therefore, False.

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Most popular questions from this chapter

What is the \(\mathrm{pH}\) of a solution whose hydronium ion concentration is \(0.0010 \mathrm{M?}\) Is the solution acidic or basic?

The \(\mathrm{pH}\) of a solution is 4 . (a) What is the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration? (b) What is the \(\mathrm{OH}^{-}\) concentration? (c) Is this solution acidic or basic?

Determine the ammonia concentration of an aqueous solution that has a pH of \(11.50\). The equation for the dissociation of \(\mathrm{NH}_{3}\) \(\left(\mathrm{K}_{\mathrm{b}}=1.8 \times 10^{-5}\right)\) is \(\mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows\) \(\mathrm{NH}_{4}^{+}(a q)+\mathrm{OH}^{-}(a q)\)

Use the Bronsted-Lowry definition to explain why \(\mathrm{NH}_{3}\) is a base in water.

It is possible to make two completely different buffers using the dihydrogen phosphate ion, \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (a) In one buffer, \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) serves as the weak acid. What is the conjugate weak base? (b) Write the equations that show how the buffer in part (a) works when either \(\mathrm{H}_{3} \mathrm{O}^{+}\) or \(\mathrm{OH}^{-}\) is added. (c) In the other buffer, \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) serves as the weak base. What is the conjugate weak acid? (d) Write the equations that show how the buffer in part (c) works when either \(\mathrm{H}_{3} \mathrm{O}^{+}\) or \(\mathrm{OH}^{-}\) is added.
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